Systems Involving Hydrogenated and Fluorinated Chains

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Systems Involving Hydrogenated and Fluorinated Chains: Volumetric Properties of Perfluoroalkanes and Perfluoroalkylalkane Surfactants Pedro Morgado,† J. Ben Lewis,‡ Carlos M. C. Laginhas,§ Luís F. G. Martins,§ Clare McCabe,‡ Felipe J. Blas,|| and Eduardo J. M. Filipe*,† †

Centro de Química Estrutural, Instituto Superior Tecnico, Universidade Tecnica de Lisboa, 1049-001 Lisboa, Portugal Department of Chemical and Biomolecular Engineering and Department of Chemistry, Vanderbilt University, Nashville, Tennessee 37235, United States § vora, Universidade de E vora, Rua Rom~ao Ramalho, 59, 7000-671 E vora, Portugal Centro de Química de E Departamento de Física Aplicada, Facultad de Ciencias Experimentales, Universidad de Huelva, 21071 Huelva, Spain

)

‡

bS Supporting Information ABSTRACT: As part of a combined experimental and theoretical study of the thermodynamic properties of perfluoroalkylalkanes (PFAAs), the liquid density of perfluorobutylpentane (F4H5), perfluorobutylhexane (F4H6), and perfluorobutyloctane (F4H8) was measured as a function of temperature from 278.15 to 353.15 K and from atmospheric pressure to 70 MPa. The liquid densities of n-perfluoropentane, n-perfluorohexane, n-perfluorooctane, and n-perfluorononane were also measured at room pressure over the same temperature range. The PVT behavior of the PFAAs was also studied using the SAFT-VR equation of state. The PFAA molecules were modeled as heterosegmented diblock chains, using different parameters for the alkyl and perfluoroalkyl segments, that were developed in earlier work. Through this simple approach, we are able to predict the thermodynamic behavior of the perfluoroalkylalkanes, without fitting to any experimental data for the systems being studied. Molecular dynamics simulations have also been performed and used to calculate the densities of the perfluoroalkylalkanes studied.

1. INTRODUCTION It is well-known that binary mixtures of alkanes and perfluoroalkanes are highly nonideal systems, in spite of the apparent similarity of the components. These mixtures exhibit large regions of liquidliquid immiscibility, large positive deviations from Raoult’s law, and large positive excess properties (such as the excess enthalpy and volume), a clear indication of weak unlike interactions. Since the late 1940s, the potential application of perfluoroalkanes as refrigerant fluids has motivated their study. In recent years, however, these substances have become key fluids in a wide range of fields due to their chemical inertness, biocompatibility, and peculiar physical properties,1,2 for example, from medical applications, where they find use as oxygen carriers in blood substitute formulations3,4 or as fluids in eye surgery, to technological applications as solvents for biphasic synthesis, fire extinguishers, or lubricants.5,6 As a result, considerable work has been carried out on the theoretical and computational modeling of n-alkane + n-perfluoroalkane mixtures717 to try and understand the nature of the unlike interaction.8,9,17 However, apart from repeatedly recognizing the need to account for large deviations to the LorentzBerthelot combining rules when estimating the unlike or cross intermolecular potential parameters, all these studies have failed to give a satisfactory explanation for the unusually weak hydrocarbonfluorocarbon interaction. r 2011 American Chemical Society

Structurally, the substitution of hydrogens for the larger and heavier fluorine atoms results in a larger cross-sectional area for fluorinated chains18 (0.283 nm2 compared to 0.185 nm2) and consequently higher densities and molar volumes for n-perfluoroalkanes when compared with n-alkanes of the same number of carbon atoms (Figure 1). These large differences in molar volume have other, subtler, consequences. For example, at 25 °C, the molar volume of n-hexane is 131.6 cm3 mol1, and that of n-perfluorohexane is almost 54% higher, 202.4 cm3 mol1. As a result, an equimolar mixture of (n-hexane + n-perfluorohexane) will have a volume fraction of n-perfluorohexane of 0.61, assuming ideality. Consequently, a probe immersed in such a mixture would “experience” a much more fluorinated environment than expected from its equimolar composition. The changes in volume that occur when mixing hydrogenated and fluorinated compounds are impressive and also deserve closer attention. For example, we have recently reported partial molar volumes at infinite dilution for a series of n-perfluoroalkanes in n-octane,19,20 and found that when a molecule of n-perfluorohexane is immersed in n-octane, at infinite dilution, its molar volume increases from 202.4 to 229.3 cm3 mol1, i.e., 13%. Received: August 7, 2011 Revised: September 20, 2011 Published: September 27, 2011 15013

dx.doi.org/10.1021/jp207567y | J. Phys. Chem. B 2011, 115, 15013–15023

The Journal of Physical Chemistry B

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Figure 1. Densities and molar volumes of n-alkanes and n-perfluoroalkanes at 298.15 K, as a function of number of carbon atoms.

Literally, a layer of empty space is created around the nperfluorohexane molecule. The effect is even more pronounced when n-alkanes are dissolved in n-perfluoroalkanes: their molar volumes increase by 20%!21 Another important difference between fluorinated and hydrogenated chains is conformational. For the n-alkanes, the value of the dihedral angle at the energy minimum of a “trans” CC bond is exactly 180°, so that the chains tend to be in their all-trans planar form. For the n-perfluoroalkanes, the dihedral angle at minimum energy is not exactly 180°, and as a consequence, perfluorinated chains display a helical conformation and rigidity, which contrasts with the flexible character of hydrogenated chains.22 It is believed that one of the consequences of chain stiffness in liquid fluorocarbons is less efficient molecular packing and the existence of “holes” in the liquid. This can explain (at least in part) the enhanced solubility of simple gases (e.g., oxygen, nitrogen, etc.) in liquid perfluoroalkanes. In summary, considerable changes in volume occur when hydrogenated chains are mixed with fluorinated chains. Furthermore, it is clear that an accurate description and interpretation of such changes should provide important information on the nature of the cross interaction between these different functional groups. Perfluoroalkylalkanes (PFAAs) are diblock compounds made up of alkyl and perfluoroalkyl segments covalently bonded to form a single chain. They can be pictured as chemical mixtures of two mutually phobic segments that in most cases would otherwise phase separate. Interesting volumetric properties can, thus, be expected for these liquids. Additionally, these molecules display the “dual character” of amphiphilic molecules and the physics of orientational ordering of smectogenic liquid crystals. Accordingly, aggregation in solvents selective for one of the blocks23,24 and smectic liquid crystalline phases have been reported for PFAAs.2527 It should be kept in mind, however, that unlike common hydrophilic/hydrophobic amphiphiles in which one of the driving forces for organization is the strong interaction between polar or ionic groups, in PFAA, the origin of the mutual segregation between alkyl and perfluoroalkyl groups,

and therefore organization, rests on the weakness of the cross interaction. This work is part of an ongoing project aiming at a detailed thermophysical characterization of liquid PFAAs. In particular, we have measured a number of properties of the pure liquids (such as liquid densities, vapor pressures, viscosities, surface tensions, and heat capacities) and mixtures (partial molar volumes at infinite dilution, water solubilities, interfacial tensions) and tried to interpret the results using equivalent information from the corresponding alkanes, perfluoroalkanes, and their mixtures. This strategy will ultimately clarify the effects of chemically linking the hydrogenated and perfluorinated segments and how this affects the properties of the new pure liquid and induces organization. Additionally, the results have been theoretically modeled with the SAFT-VR equation and PFAAs studied by computer simulation. In recent papers,19,28 we reported liquid densities as a function of temperature and pressure and partial molar volumes at infinite dilution for two PFAAs (F6H6 and F6H8). In this work we have extended the study to an additional three PFAAs: perfluorobutylpentane (F4H5), perfluorobutylhexane (F4H6), and perfluorobutyloctane (F4H8), for which partial molar volumes at infinite dilution in n-octane have also been recently reported.20 Liquid densities have been measured, at room pressure, as a function of temperature from 278.15 to 353.15 K and at 5 K intervals and from atmospheric pressure to 70 MPa. The liquid densities of n-perfluoropentane (F5), n-perfluorohexane (F6), n-perfluorooctane (F8), and n-perfluorononane (F9) were also measured at room pressure over the same temperature range. The SAFT-VR equation of state2931 has been used to model the PFAAs as diblock chains, using parameters for the alkyl and perfluoroalkyl segments developed in an earlier work.28 Through this simple approach, we are able to predict the thermodynamic behavior of the PFAAs studied, without fitting to any experimental data for the systems being studied. Additionally, the densities of the PFAAs as a function of temperature and pressure have been predicted by molecular dynamics simulation using an all-atom force field. 15014

dx.doi.org/10.1021/jp207567y |J. Phys. Chem. B 2011, 115, 15013–15023


2. EXPERIMENTAL SECTION The perfluoroalkylalkane liquids (F4H5, F4H6, and F4H8) used were ultrapurified chemicals obtained from Fluoron GMBH with a claimed purity of 100%. 19F and 1H NMR spectra of these compounds were taken in a 500 MHz Bruker spectrometer, and only very small unexpected peaks were found which, when integrated, were smaller than 1%. Hence, these compounds were used without further purification. Perfluoropentane and perfluorononane were obtained from Apollo Scientific, with 97% (85% nisomer) and 99% purity, respectively; perfluorohexane (99%) and perfluorooctane (98%) were sourced from Aldrich. All were used as received. The density measurements at ambient pressure were made in an Anton Paar DMA 5000 vibrating-tube densimeter. The instrument was calibrated with water (distilled, deionized in a Milli-Q 185 Plus water purification system and freshly boiled) and air at 20.000 °C, taking into account atmospheric pressure. The densimeter has an internal temperature control system that is stable at T ( 0.001 K. The calibration was checked with water over the whole range of operating temperatures, and the maximum deviation from literature values was found to be less than 2 105 g cm3. The cleanliness of the measurement cell was verified at the beginning of each series of measurements by checking the measured density of air. The densities at high pressure were measured in an Anton Paar DMA HP external cell, connected to the DMA 5000 densimeter. As in the DMA 5000, the temperature control is internal and stable to T ( 0.001 K; the cell was connected to a high-pressure generator and to a Setra 280E pressure transducer, which has an accuracy of 0.08 MPa. The densimeter was calibrated in vacuum over the whole range of measurement temperatures and with water, toluene, and dichloromethane in the whole range of temperature and pressure, giving a total of 737 calibration points; the average of the absolute residuals of the overall fit in relation to the literature data3234 for the calibrating fluids was 3 105 g cm3, and the individual deviations were always smaller than 2 104 g cm3. 3. MOLECULAR MODEL AND THEORY In the SAFT-VR approach, molecules are modeled as chains of tangentially bonded hard-spherical segments that interact through an attractive potential of variable range, typically a square well (SW) potential, viz. 8 > r < σ ij < þ ∞ if εij if σ ij e r < λij σij ð1Þ Uij ðrÞ ¼ > : 0 if r g λij σ ij where σij is the diameter of the interaction, λij the range, and εij the depth of the SW potential. The SAFT-VR approach has been used to successfully model the thermodynamics and phase behavior of a wide range of fluids, including alkanes, perfluoroalkanes, and their binary mixtures.14,35,36 Recently the SAFTVR approach was extended to model chain fluids composed of dissimilar segments, forming a heteronuclear rather than a homonuclear chain as in the original SAFT-VR approach and used to make predictions for the phase behavior of PFAAs and their mixtures with alkanes and perfluoroalkanes,28,30,37 as well as other fluids through a group contribution like approach.31,3840

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Table 1. Optimized SAFT-VR Parameters for the Molecules and Molecular Segments Studied segment

m

λ

σ, Å

ε/k, K

C5H11

1.998

1.505

3.931

265.0

C6H13 C8H17

2.332 2.998

1.552 1.574

3.920 3.945

250.4 250.3

C4F9

1.795

1.406

4.462

283.3

Using the heterobased SAFT-VR approach, the parameters describing the alkyl and perfluoroalkyl segments of each perfluoroalkylalkane molecule are reported in Table 1 and discussed further in the Results section. The inter- and intramolecular cross interactions between segments were obtained from the modified LorentzBerthelot combining rules8 σ ij ¼

σii þ σ jj 2

pffiffiffiffiffiffiffiffi εij ¼ ξij εii εjj λij ¼ γij

λii σ ii þ λjj σ jj σ ii þ σ jj

ð2Þ ð3Þ ð4Þ

The general form of the Helmholtz energy A within the SAFT framework is given by A Aideal Amono Achain Aassoc ¼ þ þ þ NkT NkT NkT NkT NkT

ð5Þ

We will briefly present each contribution in turn for a nonassociating fluid of diblock-heteronuclear chain molecules and direct the reader to the original references for full details of the heteroSAFT-VR approach.41,29 The ideal contribution to the Helmholtz energy is expressed as Aideal ¼ lnðFΛ3 Þ 1 NkT

ð6Þ

where N is the total number of molecules, k Boltzmann’s constant, F the number density of chain molecules, and Λ the thermal de Broglie wavelength. The monomer Helmholtz energy is given by Amono AM ¼m ¼ maM NkT Ns kT

ð7Þ

where Ns is the total number of segments, determined from the product of the total number of molecules N and the number of segments per molecule m. aM is the Helmholtz energy per monomer segment and is approximated by a second-order high-temperature expansion using Barker and Henderson perturbation theory for mixtures,42 viz. aM ¼ aHS þ βa1 þ β2 a2

ð8Þ

where β = 1/kT; aHS is the Helmholtz energy of the hard sphere reference fluid; and a1 and a2 are the first and second perturbation terms, respectively. aHS is determined from the expression of Boublik43 and Mansoori et al.44 for multicomponent hard sphere 15015



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Table 2. Experimental Densities (kg/m3) at Room Pressure, As a Function of Temperature, For the Studied Substances T/K

F5

273.15

1691.136

278.15

1675.521

1728.598

1806.278

1319.732

1288.097

1236.306

283.15

1659.678

1714.274

1793.773

1823.265

1311.591

1280.509

1229.510

288.15

1643.569

1699.762

1781.182

1811.355

1303.419

1272.913

1222.719

293.15

1627.182

1685.093

1768.496

1799.074

1295.205

1265.271

1215.899

298.15

1670.204

1755.710

1786.992

1286.961

1257.626

1209.078

303.15

1655.126

1742.819

1774.577

1278.644

1249.902

1202.221

308.15 313.15

1639.795 1624.241

1729.817 1716.678

1762.358 1749.718

1270.328 1261.909

1242.207 1234.410

1195.395 1188.486

318.15

1608.574

1703.415

1737.310

1253.493

1226.631

1181.614

323.15

1592.415

1690.000

1724.448

1244.958

1218.756

1174.665

328.15

1676.434

1711.814

1236.408

1210.873

1167.729

333.15

1662.695

1698.700

1227.757

1202.894

1160.729

338.15

1648.789

1685.806

1219.052

1194.907

1153.726

343.15

1634.681

1672.403

1210.242

1186.822

1146.657

348.15 353.15

1620.442 1605.894

1659.219 1645.677

1201.379 1192.404

1178.701 1170.494

1139.578 1132.442

F6

F8

F9

F4H5

F4H6

F4H8

Table 3. Coefficients Obtained by Fitting the Room Pressure Density Data As a Function of Temperature to Equation 12 for All Compounds Studied a0

a1

a2

F5

2150.349

26.862

51.7143

F6

2667.943

528.269

118.118

a3 17.8353

F8

2669.416

470.121

93.0836

F9

2577.846

358.068

55.3886

12.8093 8.13809

F4H5

1859.697

271.007

43.9794

5.87410

F4H6 F4H8

1778.493 1678.952

236.082 208.635

34.0669 27.2040

4.52142 3.38282

systems, while a1 is obtained from the mean-value theorem and a2 through the local compressibility approximation, as proposed by Gil-Villegas et al.45 K HS ¼

ζ0 ð1 ζ3 Þ4 ζ0 ð1 ζ3 Þ2 þ 6ζ1 ζ2 ð1 ζ3 Þ þ 9ζ32

ð9Þ

Finally, the contribution due to chain formation from the monomer segments is given in terms of the background correlation function ySW ij Achain ¼ NkT

SW ln ySW ∑ ij ðσ ij Þ ¼ expð βεij Þgij ðσ ij Þ ij bonds

ð10Þ where the sum is over all bonds in the chain molecule. For the PFAAs studied in this work, eq 10 becomes Achain ¼ ðm1 1Þln ySW 11 ðσ 11 Þ NkT SW ðm2 1Þln ySW 22 ðσ 22 Þ ln y12 ðσ 12 Þ

ð11Þ

where component one refers to the alkyl segments and two to the perfluoroalkyl segments of the PFAA. The radial distribution function for the square well monomers gSW ij (σij) is approximated

Figure 2. Comparison between the density of liquid n-perfluoroalkanes obtained in this work and data from the literature. Gray triangle, F5 from Lepori et al.;21 black triangle, F5 from Burger et al.;60 black circle, F6 from Dias et al.;61 black x, F6 from Dunlap et al.62 (air saturated liquid); black plus, F6 from Dunlap et al.62 (degassed liquid); open circle with black border, F6 from Pi~ neiro et al.;53 open circle with gray border, F6 from Kennan et al.;63 gray circle, F6 from Lepori et al.;21 black diamond, F8 from Dias et al.;64 gray diamond, F8 from Kennan et al.;63 open diamond with gray outline, F8 from Lepori et al.;21 open diamond with black outline, F8 from Mustafaev et al.;65 black square, F9 from Dias et al.;61 gray square, Pi~ neiro et al.53

by a first-order high-temperature perturbation expansion, again following the work of Gil-Villegas et al.45

4. SIMULATION DETAILS The optimized potentials for liquid simulations all-atom (OPLS-AA) force field46 with the extension to perfluoroalkanes by Watkins and Jorgensen47 has been used to describe the PFAA molecules. In the OPLS-AA force field a Lennard-Jones potential describes the intermolecular interactions and the intramolecular interactions between sites separated by three or more bonds. 15016



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Table 4. Coefficients Obtained by Fitting the Density Data As a Function of Temperature and Pressure to Equation 15 for the Three PFAAs Studied, Along with the Standard Deviation of the Fitting F4H5

F4H6 2

8.36992 10

C

8.36390 10

F4H8 2

8.34046 102

B0/MPa

320.675

329.632

345.294

B1/MPa K1

1.32734

1.34419

1.37807

B2/MPa K2

1.43613 103

1.44204 103

1.46350 103

3

F00/kg m

1720.207

F01/kg m3 K1 1.22726

1673.601

1601.261

1.23374

1.24882

F02/kg m3 K2 7.59985 104 5.42706 104 2.26929 104 σ/kg cm3 7.2 102 5.9 102 4.2 102

Figure 3. Isobaric thermal expansion coefficients at atmospheric pressure as a function of temperature for the studied substances (F6H6 and F6H8 from previous work28) and selected n-alkanes (n-hexane, n-nonane, and n-dodecane, as solid lines). F5, Δ; F6, ); F8, O; F9, 0; F4H5, (; F4H6, b; F6H6, gray circle; F4H8, 9; F6H8, gray box. The results for the n-alkanes were calculated from the density correlations of Cibulka.55

Simple geometric combining rules were used to determine the cross or unlike interactions. Bond stretching and bond angle bending are described by harmonic potentials, and torsional motion characterizing the preferred orientational and rotational barriers around all nonterminal bonds is described through the potentials of Jorgensen and Padua.48 All simulations were performed with 243 molecules in the isobaricisothermal (NpT) ensemble using the NoseHoover thermostat and barostat in the LAMMPS molecular dynamics code.49 The particleparticle particlemesh (PPPM) algorithm with a precision of 1.0 106 was used to describe the long-range electrostatic interactions and a spherical potential cut off of 12 Å used for the van der Waals interactions. All simulations were run using a time step of 1.0 fs for 2 ns, with the last 1 ns of data used to determine the density using block averaging.50

Figure 4. Isothermal compressibility coefficients at 298.15 K as a function of pressure for the studied PFAA, along with the results for selected n-alkanes (n-hexane, n-nonane, n-decane, n-dodecane, and n-tetradecane, as solid lines) and n-perfluoroalkanes. F6, ); F9, O; F4H5, 9; F4H6, b; F6H6, gray circle; F4H8, (; F6H8, gray diamond. The results for the n-alkanes were calculated from the density correlations of Cibulka.55

5. RESULTS The experimental densities as a function of temperature (at atmospheric pressure) are presented in Table 2. The results have been correlated with a simple polynomial of the form

not exceeding 1.5 and 0.75%, respectively, and are not included in the figure for simplicity. From the dependence of density with temperature, the isobaric thermal expansion coefficient

d=kg m3 ¼

n

ai ðT=100 KÞi ∑ i¼0

1 ∂F αp ¼ F ∂T p

ð12Þ

where d is the density and T the absolute temperature. The obtained coefficients allow the reproduction of the experimental values within the reproducibility of the measurements and are collected in Table 3. In the case of the n-perfluoroalkanes, the experimental results can be compared with values already available in the literature, although over a smaller temperature range as shown in Figure 2. As can be seen from the figure, our results compare favorably with the literature data, with differences that never exceed 0.5% and that are most probably due to the different sources of the perfluoroalkane samples. The exceptions are the results from Haszeldine51 and Stiles,52 which present deviations from ours

ð13Þ

can be calculated and was done by analytical differentiation of eq 12. αp coefficients for all the studied substances are recorded in Figure 3 along with data for F6H6 and F6H8, which were calculated from data obtained in previous work,28 and data for selected n-alkanes for comparison. Liquid densities for F4H5, F4H6, and F4H8 were also determined as a function of pressure. Isothermal curves were measured at 5 K intervals between 278.15 and 353.15 K, from atmospheric pressure to 70 MPa; at least 30 points were taken along each isotherm, for a total of almost 600 data points for each substance. These values were fitted with the widely used 15017



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Figure 5. Molar volumes at 298.15 K and atmospheric pressure for all the PFAA and n-perfluoroalkanes studied as a function of number of carbon atoms. Molar volumes of n-alkanes at the same conditions are also included for comparison.

modified Tait equation Fðp, TÞ ¼ F0 ðTÞ= 1 C ln

BðTÞ þ p BðTÞ þ p0

!! ð14Þ

where F0(T), C, and B(T) are the fitting parameters. F0(T) stands for the density at the reference pressure p0 = 0.101325 MPa and is given by F0(T) = Σ2i=0F0iTi. C is temperature independent, and B(T) is given by B(T) = Σ2i=0BiTi. The fitting coefficients for the three compounds are presented in Table 4, along with the standard deviation of the fit, calculated as vffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffiffi u n u u ðFexp Fcalc Þ2 ti ¼ 1 ð15Þ σ ¼ n

∑

where n is the number of experimental points. The full set of experimental data is too large to be conveniently presented in the main body of this paper and so is provided as Supporting Information. From the dependence of the density with pressure, the isothermal compressibility coefficient ! 1 ∂F ð16Þ kT ¼ F ∂p T

can be calculated. In this case, analytical differentiation of the Tait eq 14 is the most straightforward and accepted way to obtain kT.8 In Figure 4 the compressibilities at 298.15 K for the studied PFAAs are represented, together with those of F6H6 and F6H8 from previous work,28 two perfluoroalkanes from the work of Pi~ neiro et al.,53 and data for some selected alkanes, calculated from the correlations of Cibulka.54 As can be seen from the figures, perfluorocarbons are much denser than hydrocarbons but are also much more expansible and compressible. The results for the PFAAs globally show that these substances have densities, compressibilities, and expansivities between those of the n-alkanes and n-perfluoroalkanes. It can also be seen that,

when comparing substances with the same chain length, the properties of PFAAs lie closer to the corresponding n-perfluoroalkanes than to the n-alkanes.

6. DISCUSSION A global view of the results at 298.15 K and atmospheric pressure is presented in Figure 5, from which a number of interesting conclusions can be drawn. In the figure, the molar volumes of all studied PFAAs and n-perfluoroalkanes are plotted as a function of the total number of carbon atoms in the chain. Molar volumes of n-alkanes from the literature are also included for comparison. As can be seen from the figure, for the n-alkanes and n-perfluoroalkanes straight lines are obtained, the slope of which can be identified with the molar volume of the CH2 and CF2 groups, respectively, as 15.976 and 23.325 cm3 mol1. More interestingly, the molar volumes for the series (F4H5, F4H6, F4H8) also fall on a straight line. In this series, the length of the fluorinated segment is kept constant, while that of the hydrogenated segment is increased, thus the slope can be identified with the molar volume of the CH2 group when bonded to a perfluorobutyl segment (Vm(CH2)F4). As expected, the value obtained, Vm(CH2)F4 = 16.444 cm3 mol1, is 2.9% larger than the molar volume of the CH2 groups in n-alkanes, previously mentioned. Similar reasoning can be applied to the series (F6H6, F6H8), (F4H6, F6H6), and (F4H8, F6H8) yielding, respectively, Vm(CH2)F6 = 16.605 cm3 mol1, Vm(CF2)H6 = 24.87 cm3 mol1, and Vm(CF2)H8 = 25.018 cm3 mol1. The results show that, when inserted in a PFAA molecule, the molar volumes of both CH2 and CF2 groups are larger than their usual value in nalkanes and n-perfluoroalkanes and increase with the length of the hetero segment. The data are collected in Table 5. An attempt was made to interpret the results, by decomposing the molar volumes of the studied PFAAs into the molar volumes of the constituent segments, plus a volume change contribution resulting from mixing the hydrogenated and fluorinated segments and a specific term resulting from the formation of the alkylperfluoroalkyl bond. The molar volumes of the alkyl and perfluoroalkyl segments at 298.15 K can be obtained from 15018



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Table 5. Values of the Increment in Vm for CH2 and CF2 for the Three Studied Families of Compounds Vm(CH2)/

Vm(CF2)/

cm3 3 mol1

cm3 3 mol1

n-alkanes constant F4 segment

15.976 16.444

2.9%

constant F6 segment

16.605

3.9%

perfluoroalkanes

23.325

-

constant H6 segment

24.870

6.6%

constant H8 segment

25.018

7.3%

Figure 7. Contribution of the CH2CF2 junction to the molar volume of PFAA as a function of total number of carbon atoms.

Figure 6. Scheme to obtain the contribution of the CH2CF2 junction to the molar volume of F6H6.

literature data for the n-alkanes55 (molar volumes as a function of the chain length) and for the perfluoroalkanes from our own experimental data. The volume change resulting from mixing hydrogenated and fluorinated segments can be obtained from the excess volume data for several mixtures of n-alkanes and perfluoroalkanes at 298.15 K from Lepori et al.21 Finally, the contribution resulting from the existence of the alkyl perfluoroalkyl bond can be obtained by subtracting the previous two terms from the experimental molar volume. The bonding term should include contributions from several effects, namely, the presence of the dipole at the CH2CF2 junction, geometrical considerations (the cross-sectional diameter of the hydrogenated and fluorinated chains is highly incompatible relative to a close-packed arrangement. This fact contributes by itself to phase segregation. Bonding the two types of segments together will thus produce volume changes as a result of geometrical constrictions), and the reorganization of the liquid, reflecting the balance of the affinity/antipathy between the two types of segments, i.e., the building up of amphiphilic character. This procedure is illustrated in Figure 6 for F6H6. The figure clearly shows how the molar volumes for the hexyl (H6-) and perfluorohexyl (F6-) segments (which are equivalent to half the molar volumes of n-dodecane and perfluorododecane, respectively) add to obtain the volume of 2 mol of an ideal mixture of these segments (equivalent to the molar volume of an ideal mixture of (n-dodecane + perfluorododecane), Vim(H12 + F12)). Also shown are the estimated excess volumes when mixing H6and F6-segments or n-dodecane and perfluorododecane. As can be seen, these are not similar, as the excess volume depends on chain length. Finally, it is also clear that the molar volume of

F6H6 lies between Vm(H6- + F6-) and Vm(H12 + F12), although closer to the latter. This indicates that if a mixture of n-dodecane and perfluorododecane could be transformed into F6H6 by interchanging segments an increase in volume would occur. Alternatively, in a hypothetical mixture of F6- and H6- in which the segments were bonded together to form F6H6, the volume would decrease. Similar calculations were performed for all PFAAs, and the results are presented in Figure 7. As can be seen from the figure, in all cases the molar volumes of the PFAA are smaller than those of the corresponding mixtures of segments; i.e., the volume of the mixture would decrease on bonding the segments together. On the other hand, the molar volumes of four of the studied PFAAs are larger than those of the corresponding mixture of alkanes and perfluoroalkanes; i.e., an increase of the molar volume would occur on interchanging segments. The molar volume of F4H5, however, is slightly smaller than that of an equimolar mixture of n-decane and perfluorooctane; that is, a volume contraction would occur in this case, either by bonding together the constituent segments or by interchanging segments between the parent molecules. Furthermore, in either case, the differences found contain the volume contribution of the CH2CF2 bond. As can be seen, these are not constant but increase with the total chain length of the PFAA molecules in a similar way, reflecting that they are different ways of expressing the same physical feature. The results obtained for the PFAAs studied have been interpreted using two theoretical approaches: molecular dynamics simulations and the SAFT-VR equation of state. Liquid densities were obtained from molecular dynamics simulations for F4H5, F4H6, and F4H8 as a function of temperature and pressure and as a function of temperature only, for F6H6 and F6H8. Liquid densities were also calculated for F5H5 and found to be in excellent agreement with the simulations of Pierce et al.56 The results are presented in Table 6 and plotted in Figure 8, from which a number of conclusions can be drawn. As can be seen from the figure, the simulations are able to predict the liquid densities in excellent agreement with the experimental results. Globally, the deviations lie between 2.4 and 1.4%, which are well within those usually found for 15019



ARTICLE

Table 6. Simulation Results for the Liquid Density of PFAA, at Different Temperatures and Pressures and Comparison with Experimental Results density (kg 3 m3) F4H5 p = 0.101325 MPa

p = 25.33125 MPa

Table 6. Continued p = 50.66250 MPa T/K

simulation

experiment

dev. (%)

313 333

1256 ( 3 1232 ( 3

1254.20 1233.40

0.2 0.1

353

1208 ( 4

1213.03

0.4

T/K simulation experiment dev. (%) simulation experiment dev. (%) 278 1314 ( 6

1320.29

0.5

1357 ( 5

1358.72

0.1

298 1273 ( 4

1286.99

1.1

1323 ( 3

1330.51

0.6

313 1246 ( 7

1261.62

1.3

1300 ( 4

1309.53

0.7

F6H6

F6H8

p = 0.101325 MPa

p = 0.101325 MPa

T/K simulation experiment dev. (%) simulation experiment dev. (%)

333 1205 ( 6

1227.25

1.8

1268 ( 4

1281.86

1.1

278 1427 ( 6

1418.32

0.6

1371 ( 4

1360.38

0.8

353 1164 ( 7

1192.28

2.4

1237 ( 6

1254.54

1.4

298 1387 ( 4 313 1357 ( 5

1386.33 1362.15

0.0 0.4

1345 ( 5 1314 ( 4

1330.97 1308.93

1.1 0.4

p = 50.66250 MPa

333 1319 ( 7

1329.48

0.8

1274 ( 5

1279.04

0.4

353 1284 ( 5

1296.11

0.9

1244 ( 4

1249.40

0.4

T/K

simulation

experiment

dev. (%)

278 298

1386 ( 3 1359 ( 4

1388.99 1363.70

0.2 0.3

313

1338 ( 3

1345.08

0.5

333

1310 ( 4

1320.75

0.8

353

1284 ( 4

1296.90

1.0

F4H6 p = 0.101325 MPa

p = 25.33125 MPa


1288.67

0.2

1324 ( 5

1323.84

0.0

298 1252 ( 5

1257.75

0.4

1294 ( 4

1297.39

0.2

313 1224 ( 5

1234.27

0.9

1272 ( 3

1277.73

0.4

333 1187 ( 4

1202.59

1.3

1243 ( 4

1251.82

0.7

353 1149 ( 6

1170.46

1.8

1213 ( 4

1226.23

1.1

p = 50.66250 MPa T/K

simulation

experiment

278

1354 ( 3

1351.90

0.1

298 313

1326 ( 3 1306 ( 4

1328.08 1310.56

0.2 0.3

333

1280 ( 4

1287.65

0.6

353

1256 ( 4

1265.19

0.7

dev. (%)

F4H8 p = 0.101325 MPa

p = 25.33125 MPa


1236.55

0.8

1284 ( 4

1267.06

1.4

298 1215 ( 5

1208.96

0.5

1251 ( 4

1243.10

0.6

313 1185 ( 4

1188.15

0.2

1228 ( 4

1225.36

0.2

333 1155 ( 4

1160.24

0.5

1200 ( 4

1202.03

0.2

353 1120 ( 6

1132.22

1.1

1170 ( 5

1179.04

0.7

p = 50.66250 MPa T/K

simulation

experiment

278

1309 ( 4

1291.85

1.3

298

1280 ( 3

1270.14

0.8

dev. (%)

pure n-alkanes and n-perfluoroalkanes. In most cases, the simulations predict densities slightly lower than the experimental, except for the heaviest PFAA at the lowest temperatures, but slightly overpredict the expansivity of all liquids. Moreover, for the three PFAAs studied in this work, the agreement between experimental and simulated densities improves at higher pressures. It should be emphasized that the simulations were done using simple geometrical combining rules to obtain the cross interaction parameters. Song et al.17 have shown that for binary mixtures of n-alkanes + n-perfluoroalkanes the reduction of the FH cross interaction by 25% changes significantly the enthalpy of mixing, bringing it close to the experimental results, but has little effect on the density, showing that this property is not very sensitive to small changes in the interactions. This behavior is also observed for the PFAAs studied, though to elucidate this point further it would be important to simulate other properties of PFAAs, namely, vapor pressures and vaporization enthalpies, and this will be done in future work. Additionally, the F4H5, F4H6, and F4H8 liquids have been modeled with the hetero-SAFT-VR equation using a totally predictive approach. The number of spherical segments forming the alkyl and perfluoroalkyl chains was determined as in the previous paper of this series,28 giving the values of 1.997, 2.332, 2.998, and 1.795 for pentyl, hexyl, octyl, and perfluorobutyl segments, respectively. The square-well parameters ε, σ, and λ for the alkyl and perfluoroalkyl chains and the binary interaction parameters that mediate the strength of the cross interaction (ξij = 0.840 and γij = 1.0451) were all taken from earlier work on the alkanes and perfluoroalkanes.5759 The results of the hetero-SAFT-VR predictions for the molar volume of all the PFAA compounds (the three studied here and the two studied in the previous work) at a pressure of 1 atm are presented in Figure 9, along with the corresponding experimental results. It can be seen that, although the expansivity is overpredicted by the theory, the error in the molar volumes compared to the experimental data is always less than 1%. This agreement is remarkable, especially considering that the theoretical results are true predictions, since no parameters were fitted to experimental data for the fluids being studied. SAFT-VR calculations were also performed to predict the molar volumes of F4H5, F4H6, and F4H8 as a function of 15020



ARTICLE

Figure 8. Comparison between experimental (lines) and simulated (points) densities as a function of temperature for: (a) F4H5 (b, 0.101325 MPa; Δ, 25.33125 MPa; 9, 50.6625 MPa); (b) F4H6 (idem); (c) F4H8 (idem); (d) b, F6H6; O, F6H8 at 0.101325 MPa.

Figure 9. Comparison between experimental and SAFT-VR results of molar volume at atmospheric pressure as a function of temperature for five PFAAs. Experimental results: (, F4H5; b, F4H6; 9, F4H8; O, F6H6; 0, F6H8. SAFT-VR predictions: lines.

pressure. The results for F4H8 are presented in Figure 10, along with the experimental data. From the figure, it can be seen that the theory overpredicts the compressibility since the slope of the theoretical curves is considerably larger than that of the experimental results; however, if a comparison is made directly between the predicted molar volumes and the experimental data, the error is

Figure 10. Comparison between experimental and SAFT-VR results of molar volume for F4H8 as a function of pressure at eight temperatures (from 278.15 to 348.15 K with intervals of 10 K). Points: experimental results. Lines: SAFT-VR predictions.

smaller than 3.5%, even at 600 bar. The results for the other PFAAs studied show similar behavior and so are not shown.

’ CONCLUSIONS The liquid density of perfluorobutylpentane (F4H5), perfluorobutylhexane (F4H6), and perfluorobutyloctane (F4H8) 15021


The Journal of Physical Chemistry B was measured as a function of temperature from 278.15 to 353.15 K and from atmospheric pressure to 70 MPa. The liquid density of n-perfluoropentane, n-perfluorohexane, n-perfluorooctane, and n-perfluorononane was also measured at room pressure, in the same temperature range. The results indicate that the molar volume of PFAAs is larger than that of mixtures of (n-alkanes + perfluoroalkanes) with similar chain length. The results were further interpreted using the hetero-SAFTVR equation of state. The perfluoroalkylalkanes were modeled as heterosegmented diblock chains, using parameters for the alkyl and perfluoroalkyl segments developed in earlier work. This fully predictive approach is able to estimate the liquid density of the perfluoroalkylalkanes at atmospheric pressure within 1% and at pressures up to 600 MPa within 3.5% without fitting to any experimental data for the PFAAs. Finally, molecular dynamics simulations were performed using an atomistically detailed force field. The deviations between the simulated densities and experimental data lie between 2.4 and 1.4% for all the PFAAs studied and are comparable to those found for pure n-alkanes and n-perfluoroalkanes. In this case, the cross interaction parameters were taken as the geometric mean of the pure parameters; deviation from the geometric mean value was not needed to predict accurate PVT behavior. The ability of the OPLS all-atom force field to predict other physical properties of the PFAAs will be investigated in future work.

’ ASSOCIATED CONTENT

bS

Supporting Information. Supporting Tables 13. This material is available free of charge via the Internet at http://pubs. acs.org.

’ ACKNOWLEDGMENT P.M. acknowledges funding from Fundac-~ao para a Ciência e Tecnologia, in the form of a PhD grant (No. SFRH/BD/39150/ 2007). E.J.M.F. acknowledges funding from the Fundac-~ao para Ciência e Tecnologia through grant numbers POCI/QUI/ 61850/2004 and PEst-OE/QUI/UI0100/2011. C.M.C. and J.B.L. acknowledge support from the Office of Naval Research under grant numbers N00014-06-1-0624, N00014-09-1-0334. and N00014-09-10793 and gratefully acknowledge the National Energy Research Scientific Computing Centre, which is supported by the Office of Science of the Department of Energy under Contract No. DE-AC02-05CH11231, for computational resources. C.M.C. also acknowledges support from the Jacob Wallenberg Foundation and the National Science Foundation through grant numbers CTS-0829062 and CBET-1067642. L.F.G.M. acknowledges funding from Fundac-~ao para a Ciência e Tecnologia through grant POCTI/QUI/46299/2002. F.J.B. is grateful for financial support from project numbers FIS201014866 of the Spanish DGICYT (Direccion General de Investigacion Científica y Tecnica) and HP2005-045 of the Spanish MEC (Ministerio de Educacion y Ciencia, Programa de Acciones Integradas), as well as for additional financial support from Universidad de Huelva and Junta de Andalucía. ’ REFERENCES (1) (2) (3) (4)

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Systems Involving Hydrogenated and Fluorinated Chains

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